CHEMISTRY Practice Exam #2
|
|
- Ashlynn James
- 5 years ago
- Views:
Transcription
1 CHEMISTRY Practice Exam #2 Section 1 - This section of the exam is multiple choice. Choose the BEST answer from the choices which are given. 1. Which of the following solutions will have the highest concentration of chloride ions? A M NaCl B M MgCl2 C M AlCl3 D M CaCl2 2. How many milliliters of a 9.0 M H2SO4 solution are needed to make 0.35 L of a 3.5 M solution? A ml B ml C. 140 ml D. 900 ml 3. Identify HCl. A) strong electrolyte, weak acid B) weak electrolyte, weak acid C) strong electrolyte, strong acid D) weak electrolyte, strong acid 4. Identify NaCl. A) weak acid B) weak electrolyte C) strong acid D) strong electrolyte 5. Which of the following pairs of aqueous solutions will form a precipitate when mixed? A) NH4NO3 + Li2CO3 B) Hg2(NO3)2 + LiI C) NaCl + Li3PO4 D) AgC2H3O2 + Cu(NO3)2 6. Identify the spectator ions in the following molecular equation. KBr(aq) + AgNO3(aq) AgBr(s) + KNO3(aq) A) Ag+ and Br- B) K+ and NO3 - C) K+ and Br- D) Ag+ and NO3 -
2 7. Give the net ionic equation for the reaction that occurs when aqueous solutions of H2SO4 and KOH are mixed. A) H+(aq) + OH-(aq) H2O(l) B) 2 K+(aq) + SO4 2- (aq) K2SO4(s) C) H+(aq) + OH-(aq) + 2 K+(aq) + SO4 2- (aq) H2O(l) + K2SO4(s) D) H2 2+ (aq) + OH-(aq) H2(OH)2(l) 8. The titration of 25.0 ml of an unknown concentration H2SO4 solution requires 83.6 ml of 0.12 M LiOH solution. What is the concentration of the H2SO4 solution (in M)? A) 0.20 M B) 0.40 M C) 0.10 M D) 0.36 M 9. Which of the following is an acid base reaction? A) C(s) + O2(g) CO2(g) B) 2 HClO4(aq) + Ca(OH)2(aq) 2 H2O(l) + Ca(ClO4)2(aq) C) Fe(s) + 2 AgNO3(aq) 2 Ag(s) + Fe(NO3)2(aq) D) MgSO4(aq) + Ba(NO3)2(aq) Mg(NO3)2(aq) + BaSO4(s) 10. Determine the oxidation state of Sn in Sn(SO4)2. A) +2 B) +4 C) +6 D) What element is undergoing oxidation (if any) in the following reaction? Zn(s) + 2 AgNO3(aq) Zn(NO3)2(aq) + 2 Ag(s) A) Zn B) N C) O D) Ag 12. What is the oxidation number change for the bromine atom in the following unbalanced reduction half reaction: BrO 3 - (aq) + H + (aq) Br - (aq) + I A) -7 B) - 6 C) + 6 D) + 7
3 13. Which of the following signs on q and w represent a system that is doing work on the surroundings, as well as gaining heat from the surroundings? A) q = +, w = - B) q = -, w = + C) q = +, w = + D) q = -, w = Calculate the change internal energy (ΔE) for a system that is giving off 45.0 kj of heat and is performing 855 J of work on the surroundings. A) 44.1 kj B) kj C) kj D) 9.00 x 102 kj 15. A sample of copper absorbs 43.6 kj of heat, resulting in a temperature rise of 75.0 C, determine the mass (in kg) of the copper sample if the specific heat capacity of copper is J/g C. A) 1.51 kg B) 6.62 kg C) 1.26 kg D) 7.94 kg 16. The specific heat capacity of liquid water is 4.18 J/g-K. How many joules of heat are needed to raise the temperature of 5.00 g of water from 25.1 C to 65.3 C? A) 48.1 J B) 840 J C) J D) J 17. Which of the following substances (with specific heat capacity provided) would show the greatest temperature change upon absorbing J of heat? A) 10.0 g Fe, CFe = J/g C B) 10.0 g H2O, CH2O = 4.18 J/g C C) 10.0 g ethanol, Cethanol = 2.42 J/g C D) 10.0 g Au, CAu = J/g C 18. How much energy is evolved during the reaction of 48.7 g of Al, according to the reaction below? Assume that there is excess Fe2O3. Fe2O3(s) + 2 Al(s) Al2O3(s) + 2 Fe(s) ΔH rxn = -852 kj A) 415 kj B) 769 kj C) 241 kj D) 130 kj
4 19. Use the standard reaction enthalpies given below to determine ΔH rxn for the following reaction: 2 NO(g) + O2(g) 2 NO2(g) ΔH rxn =? Given: N2(g) + O2(g) 2 NO(g) ΔH rxn = +183 kj 1/2 N2(g) + O2(g) NO2(g) ΔH rxn = +33 kj A) kj B) -117 kj C) -333 kj D) +115 kj 20. Choose the reaction that illustrates ΔH f for NaHCO3. A) Na(s) + H2(g) + C(s) + O2(g) NaHCO3 (s) B) Na+(aq) + HCO3-1 (aq) NaHCO3 (s) C) Na+(aq) + H2O (l) + CO2 (g) NaHCO3 (s) D) Na(s) + 1/2 H2(g) + C(s) + 3/2 O2(g) NaHCO3 (s) 21. Use the information provided to determine ΔH rxn for the following reaction: ΔH f (kj/mol) CH4(g) + 3 Cl2(g) CHCl3(l) + 3 HCl(g) ΔH rxn =? CH4(g) -75 CHCl3(l) -134 HCl(g) -92 A) -151 kj B) -335 kj C) +662 kj D) +117 kj 22. To what temperature must a balloon, initially at 25 C and 2.00 L, be heated in order to have a volume of 6.00 L? A) 993 K B) 403 K C) 75 K D) 894 K 23. How many moles of CO are contained in a 5.00 L tank at 155 C and 2.80 atm? A) moles B) 1.10 moles C) 2.51 moles D) moles
5 24. What is the volume of 5.60 g of O2 at 7.78 atm and 415K? A) 1.53 L B) 565 L C) 24.5 L D) L 25. Which of the following samples will have the greatest volume at STP? A) 22 g CO B) 22 g He C) 22 g O2 D) 22 g Cl2 26. Place the following gases in order of increasing density at STP. N2 NH3 N2O4 Ar A) N2O4 < Ar < N2 < NH3 B) Ar < N2O4 < N2 < NH3 C) NH3 < Ar < N2 < N2O4 D) NH3 < N2 < Ar < N2O4 27. The density of a gas is 1.43 g/l at STP. What is the gas? A) Cl2 B) S C) O2 D) Ne 28. A g sample of an unknown gas occupies 245 ml at 298 K and 1.22 atm. What is the molar mass of the unknown compound? A) 26.3 g/mol B) 33.9 g/mol C) 12.2 g/mol D) 38.0 g/mol 29. The heat of vaporization of water at 100 C is kj/mol. Calculate the quantity of heat that is absorbed/released when 9.00 g of steam condenses to liquid water at 100 C. A) 20.3 kj of heat are absorbed. B) 20.3 kj of heat are released. C) 81.3 kj of heat are absorbed. D) 81.3 kj of heat are released. 30. Calculate the total quantity of heat required to convert 25.0 g of liquid CCl4(l) from 35.0 C to gaseous CCl4 at 76.8 C (the normal boiling point for CCl4). The specific heat of CCl4(l) is J/(g C), its heat of fusion is 3.27 kj/mol, and its heat of vaporization is kj/mol. A) kj B) 1.43 kj C) 5.74 kj D) 6.28 kj
6 Section 2 - Calculations Involving Chemical Equations Consider the following reaction BaCl 2 (s) + H 2 SO 4 (l) > BaSO 4 (s) + 2 HCl (g) A mixture of 2.65 g of BaCl 2 and 6.78 g of H 2 SO 4 are allowed to react. Molar masses: BaCl 2, H 2 SO 4, BaSO 4, HCl, How many grams of BaSO 4 could theoretically be produced from the 2.65 g of BaCl 2? 2.97 Answer: g 2. How many grams of BaSO 4 could theoretically be produced from 6.78 g of H 2 SO 4? c) Which is the limiting reagent in this reaction? 16.1 Answer: g Answer: d) If 1.25 g of BaSO 4 is actually isolated, what is the percentage yield for the reaction? BaCl2 42.1% Answer:
7 3 - Calculations involving Solutions 1. Calculate the molarity of a solution prepared by dissolving g of LiOH in enough water to give a final volume of 750. ml (Show work.) (1.495 g LiOH) x (1 mol/23.95 g LiOH) = mol LiOH ( mol LiOH)/(0.750 L) = M 2. Describe how you would prepare ml of M NaCl (M = g/mol) from solid NaCl. (.2500 L soln) x (3.000 mol/1.000 L soln) x (58.45 g NaCl/1 mol NaCl) = g NaCl g NaCl is dissolved in enough water to make ml.
8 Section 4 - Follow the directions to solve each problem. 1. An unknown liquid is vaporized in a 273-mL flask by immersion in a water bath at 99 C. The barometric pressure is 753 torr. If the mass of the liquid retained in the flask is g, what is its molar mass? a. Find the number of moles of gas present using the ideal gas law..009 moles b. Using the measured mass of the liquid, find its molar mass. 150 g/mol 2. A small quantity of hydrogen was prepared by the addition of hydrochloric acid to zinc. 195 ml of hydrogen was collected over water at 25 C and 753 torr. from the reaction. (Pwater = 24 torr at 25 C) a. Write the balanced chemical equation for the reaction of zinc metal with hydrochloric acid to yield zinc chloride and hydrogen gas. Zn (s) + 2 HCl (aq)----> ZnCl2 (aq) + H2 (g) b. Correcting for water vapor pressure, what was the pressure of the hydrogen gas collected? 729 torr c. Using the ideal gas equation, calculate the number of moles of hydrogen gas collected? moles d. How many grams of zinc were present in the original reaction?.500 g
CHEMISTRY Practice Exam #2 (KATZ)
CHEMISTRY 1710 - Practice Exam #2 (KATZ) Section 1 - This section of the exam is multiple choice. Choose the BEST answer from the choices which are given and write the letter for your choice in the space
More informationCHEMISTRY Practice Exam #2 (KATZ)
CHEMISTRY 1710 - Practice Exam #2 (KATZ) Section 1 - This section of the exam is multiple choice. Choose the BEST answer from the choices which are given and write the letter for your choice in the space
More informationCHEMISTRY Practice Exam #2 -Answers (KATZ)
HEMISTRY 1710 - Practice Exam #2 -Answers (KATZ) Section 1 - This section of the exam is multiple choice. hoose the EST answer from the choices which are given and write the letter for your choice in the
More informationCHEMISTRY Practice Exam #3 - SPRING 2013
CHEMISTRY 1710 - Practice Exam #3 - SPRING 2013 Section 1 - This section of the exam is multiple choice. Choose the BEST answer from the choices which are given and write the letter for your choice in
More informationChemistry: A Molecular Approach (Tro) Chapter 4. Chemical Quantities and Aqueous Reactions
Chemistry: A Molecular Approach (Tro) Chapter 4 Chemical Quantities and Aqueous Reactions 1) According to the following balanced reaction, how many moles of NO are formed from 8.44 moles of NO 2 if there
More informationReview Exam 2. 2.What is the mass of 4 atom(s) of copper in grams? A) g B) g C) g D) g E) 4.
Review Exam 2 1.Naturally occurring element X exists in three isotopic forms: X-28 (27.977 amu, 92.23% abundance), X-29 (28.976 amu, 4.67% abundance), and X-30 (29.974 amu, 3.10% abundance). Calculate
More informationCHE105 SU17 Exam 2. Question #: 1. Question #: 2
CHE105 SU17 Exam 2 Your Name: Your ID: Question #: 1 The percent yield of a reaction is 68.9%. What is the actual yield for this reaction, if the theoretical yield is 26.0 grams? Actual yield = 1 g Report
More informationMULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question.
Exam Name MULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question. 1) When the following equation is balanced, the coefficients are. 1) NH3 (g) + O2 (g) NO2
More informationCHE 105 Exam 2 Fall 15
CHE 105 Exam 2 Fall 15 Question #: 1 Which of the following statements is(are) true for ionic bonds? Select all that apply. A. These bonds typically form between a metal and a nonmetal. B. The formation
More informationb) Na 2 S(aq) + ZnCl 2 (aq) ZnS(s) + 2 NaCl(s)
Chem 111 2010 Name: Vining Exam #2, Version 23 1. Which of the following compounds are soluble in water: K 2 CO 3, CaCO 3, NiCO 3, and Fe 2 (CO 3 ) 3? a) K 2 CO 3 only b) K 2 CO 3 and CaCO 3 c) CaCO 3
More informationName: Thermochemistry. Practice Test C. General Chemistry Honors Chemistry
Name: Thermochemistry C Practice Test C General Chemistry Honors Chemistry 1 Objective 1: Use the relationship between mass, specific heat, and temperature change to calculate the heat flow during a chemical
More informationMULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question.
Exam #2 version A Name MULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question. 1) In which species does sulfur have the highest oxidation number? A) S8 (elemental
More informationGENERAL CHEMISTRY I CHEM SYSTEM FINAL EXAM VERSION A Fall 2016
GENERAL CHEMISTRY I CHEM 1411 SYSTEM FINAL EXAM VERSION A Fall 2016 Departmental Final Exam General Chemistry I, CHEM 1411 Fall 2016 VERSION A Part I: 35 Multiple Choice (2 pts each). Directions: Select
More informationCH 221 Sample Exam Exam II Name: Lab Section:
Exam II Name: Lab Section: Part I: Multiple Choice Questions (100 Points) Use a scantron sheet for Part I. There is only one best answer for each question. 1. When methanol undergoes complete combustion,
More informationThermochemistry HW. PSI Chemistry
Thermochemistry HW PSI Chemistry Name Energy 1) Objects can possess energy as: (a) endothermic energy (b) potential energy A) a only B) b only C) c only D) a and c E) b and c (c) kinetic energy 2) The
More informationCHM 2045, Fall 2016, Final Exam Review Packet
Study Tips for the Final: - WRITE OUT EVERYING (This is the easiest way to prevent silly mistakes and the easiest way to find them!) - Make note of you frequent mistakes! (Correct molar mass? Units? SI
More information(B) K2O potassium dioxide
PRACTICE CHEMISTRY EOC TEST 1. Which substance is a conductor of electricity? (A) NaCl(s) (B) NaCl(l) (C) C6H12O6(s) (D) C6H12O6(l) 2. Which formula is correctly paired with its name? (A) MgCl2 magnesium
More informationTopic 1: Quantitative Chemistry (Stoichiometry)12.5hr
Topic 1: Quantitative Chemistry (Stoichiometry)12.5hr 1.1 The Mole, Mass, & Avogadro s constant (number) Introduction mole the amount of a substance that contains the same number of particles as the number
More informationCHE 105 FA17 Exam 2. How many moles of beryllium are in 15.0 grams of Be?
CHE 105 FA17 Exam 2 Your Name: Your ID: Question #: 1 How many moles of beryllium are in 150 grams of Be? A 66 B 13515 C 901 D 0601 Question #: 2 Vanillin, C8H8O3, is the molecule responsible for the vanilla
More informationChemistry 212 Fall 2017 Exam III - A
Chemistry 212 Fall 2017 Exam III - A Name MULTIPLE CHOICE. (1 point each) Choose the one alternative that best completes the statement or answers the question. 1) An important step in the synthesis of
More informationName. Practice Test 2 Chemistry 111
Name Practice Test 2 Chemistry 111 1) In the aqueous reaction of K 2 SO 4 (aq) + Ba(NO 3 ) 2 (aq) BaSO 4 (s) + 2KNO 3 (aq), which ions are the spectator ions? A) Ba 2+ 2- and SO 4 B) Ba 2+ and K + C) Ba
More informationName Date Class SECTION 16.1 PROPERTIES OF SOLUTIONS
SOLUTIONS Practice Problems In your notebook, solve the following problems. SECTION 16.1 PROPERTIES OF SOLUTIONS 1. The solubility of CO 2 in water at 1.22 atm is 0.54 g/l. What is the solubility of carbon
More informationtemperature change a) On heating, solid calcium carbonate yields solid calcium oxide and gaseous carbon dioxide. 4Li(s) + O2(g) 2Li2O(s)
CHEMISTRY WKST CH. 7 & 8 REVIEW (REACTIONS & EQUATIONS) NAME: JMS 1) What are the 5 evidences that a chemical reaction took place? precipitate forms color change gas released temperature change 2) Consider
More informationCHEMISTRY CP Name: Period:
CHEMISTRY CP Name: Period: CHEMISTRY SPRING FINAL REVIEW SHEET NOTE: Below are concepts that we have covered in class throughout the second semester. Questions are organized by chapter/concept to help
More informationCHE 105 Fall 16 - Exam 2
CHE 105 Fall 16 - Exam 2 Your Name: Your ID: Question #: 1 Calculate the number of atoms in a 4.54 g sample of CH4. A. 25 B. 8.52 10 23 C. 2.27 10 23 D. 0.295 Question #: 2 What is the name of BaCl2? 1
More information8. A piece of Mg(s) ribbon is held in a Bunsen burner flame and begins to burn according to the equation: 2Mg(s) + O2 (g) 2MgO(s).
1. Which event must always occur for a chemical reaction to take place? A) formation of a precipitate B) formation of a gas C) effective collisions between reacting particles D) addition of a catalyst
More informationGeneral Chemistry Study Guide
General Chemistry 1311 Study Guide Name : Louise K number: Date: Oct 02006 Instructor: Jingbo Louise Liu kfjll00@tamuk.edu 1 Chapter 04 & 05 (10 questions required and 5 questions for extra credit) Credited
More informationCHEMISTRY 110 EXAM 3 April 2, 2012 FORM A 1. Which plot depicts the correct relationship between the volume and number of moles of an ideal gas at constant pressure and temperature? 2. The height of the
More informationSlide 1 / Objects can possess energy as: (a) endothermic energy (b) potential energy (c) kinetic energy. a only b only c only a and c b and c
Slide 1 / 84 1 Objects can possess energy as: (a) endothermic energy (b) potential energy (c) kinetic energy A B C D E a only b only c only a and c b and c Slide 2 / 84 2 The internal energy of a system
More informationPractice Packet Unit 7: Moles & Stoichiometry
PRACTICE PACKET: Unit 7 Moles & Stoichiometry Regents Chemistry: Practice Packet Unit 7: Moles & Stoichiometry Vocabulary: Lesson 1: Lesson 6: Lesson 2: Lesson 4A: Lesson 4B: Lesson 3: Lesson 5: www.chempride.weebly.com
More information1. Determine the mass of water that can be produced when 10.0g of hydrogen is combined with excess oxygen. 2 H 2 + O 2 2 H 2 O
Pre-AP Chemistry Spring 2016 Final Review Objective 6.1: Students will recognize indicators of chemical change write balanced chemical equations to describe them based on common reactivity patterns. [S.12.C.1,
More informationCHEMISTRY - ZUMDAHL 2E CH.6 - TYPES OF CHEMICAL REACTIONS AND SOLUTION STOICHIOMETRY
!! www.clutchprep.com CONCEPT: MOLARITY Molarity (M) can serve as the connection between the interconversion of to and vice versa. For example, a 5.8 M NaCl solution really means per. ( Molarity = MolesSolute
More information1.1 Introduction to the Particulate Nature of Matter and Chemical Change MATTER. Homogeneous (SOLUTIONS)
TOPIC 1: STOICHIOMETRIC RELATIONS 1.1 Introduction to the Particulate Nature of Matter and Chemical Change MATTER Mass Volume Particles Particles in constant motion MATTER Pure Matters Mixtures ELEMENTS
More informationB 2 Fe(s) O 2(g) Fe 2 O 3 (s) H f = -824 kj mol 1 Iron reacts with oxygen to produce iron(iii) oxide as represented above. A 75.
1 2004 B 2 Fe(s) + 3 2 O 2(g) Fe 2 O 3 (s) H f = -824 kj mol 1 Iron reacts with oxygen to produce iron(iii) oxide as represented above. A 75.0 g sample of Fe(s) is mixed with 11.5 L of O 2 (g) at 2.66
More information(E) half as fast as methane.
Name AP Chem / / AP Chem Practice Exam #2 Part I: 40 Questions, 40 minutes, Multiple Choice, No Calculator Allowed Bubble the correct answer on the BLUE SIDE of your scantron for each of the following.
More informationCHEM 1411 Zumdahl & Zumdahl PRACTICE EXAM II (Chapters 4, 5, 6)
CHEM 1411 Zumdahl & Zumdahl PRACTICE EXAM II (Chapters 4, 5, 6) Multiple Choices: Select one best answer. 1. Which of the following is a weak electrolyte? (a) barium hydroxide solution (b) ammonia solution
More informationChapter 10 Practice. Name: Multiple Choice Identify the choice that best completes the statement or answers the question.
Name: Score: 0 / 18 points (0%) [3 open ended questions not graded] Chapter 10 Practice Multiple Choice Identify the choice that best completes the statement or answers the question. 1. A sample of gas
More informationCh 10 Practice Problems
Ch 10 Practice Problems 1. Which of the following result(s) in an increase in the entropy of the system? I. (See diagram.) II. Br 2(g) Br 2(l) III. NaBr(s) Na + (aq) + Br (aq) IV. O 2(298 K) O 2(373 K)
More information1. Rank the following elements in order of increasing atomic radius: P, Al, Cl, F, S
Useful constants and other information: R = 0.0821 LCatm/KCmole R = 8.314 J/KCmole h = 6.626 x 10-34 JCs 1 atm = 760 torr Specific heat of H 2 O(l) = 4.184 J/gC C 1 cal = 4.184 J c = 3 x 10 8 m/s PART
More informationBe able to derive chemical equations from narrative descriptions of chemical reactions.
CHM 111 Chapter 4 Worksheet and Study Guide Purpose: This is a guide for your as you work through the chapter. The major topics are provided so that you can write notes on each topic and work the corresponding
More informationFinal Exam Review-Honors Name Period
Final Exam Review-Honors Name Period This is not a fully comprehensive review packet. This packet is especially lacking practice of explanation type questions!!! You should study all previous review sheets
More informationChapter 19 Chemical Thermodynamics
Chapter 19. Chemical Thermodynamics Sample Exercise 19.2 (p. 819) Elemental mercury is a silver liquid at room temperature. Its normal freezing point is -38.9 o C, and its molar enthalpy of fusion is H
More information15.0 g Fe O 2 mol Fe 55.8 g mol Fe = g
CHAPTER Practice Questions.1 1 Mg, O, H and Cl (on each side).. BaCl (aq) + Al (SO ) (aq) BaSO (s) + AlCl (aq).5 0.15 mol 106 g mol 1 = 1. g 15.0 g Fe O mol Fe 55.8 g mol Fe = 10.9 g 1 159.7 g mol FeO
More information(1) M (2) M (3) M (4) M
Form Code A CHM 2045, Fall 2018 NAME Final Exam Review (Sumner, Gower, Korolev, Angerhofer, Polanco) Instructions: On your Scantron form, enter and bubble your name, UFID, and Form Code (see above). Turn
More informationCHEMISTRY - CLUTCH CH.4 - CHEMICAL QUANTITIES & AQUEOUS REACTIONS
!! www.clutchprep.com CONCEPT: MOLARITY Molarity (M) can serve as the connection between the interconversion of to and vice versa. For example, a 5.8 M NaCl solution really means per. ( Molarity = MolesSolute
More informationHomework 02 - Ideal Gases
HW02 - Ideal Gases This is a preview of the draft version of the quiz Started: Aug 8 at 4:48pm Quiz Instructions Homework 02 - Ideal Gases Question 1 A gas is enclosed in a 10.0 L tank at 1200 mmhg pressure.
More informationReview Material for Exam #2
Review Material for Exam #2 1. a. Calculate the molarity of a solution made with 184.6 mg sample of potassium dichromate dissolved in enough water to give 500.0 ml of solution. b. What is the molarity
More informationLesson (1) Mole and chemical equation
Lesson (1) Mole and chemical equation 1 When oxygen gas reacts with magnesium, magnesium oxide is formed. Such Reactions are described by balanced equations known as "chemical equations" Δ 2Mg(s) + O2(g)
More informationNOTE: This practice exam contains more than questions than the real final.
NOTE: This practice exam contains more than questions than the real final. 1. The wavelength of light emitted from a green laser pointer is 5.32 10 2 nm. What is the wavelength in meters? 2. What is the
More informationChapter 5 Practice Multiple Choice & Free
Name Response 1. A system has an increase in internal energy, E, of 40 kj. If 20 kj of work, w, is done on the system, what is the heat change, q? a) +60 kj d) -20 kj b) +40 kj e) -60 kj c) +20 kj 2. Which
More informationa. 36.9% b. 2.67% c. 50.4% d. 20.7% e. 12.7% 2. What is the atomic symbol for an element with 39 protons and 50 neutrons?
Name: Lab Section: Use a scantron to complete the exam. There is only one best answer for each question. Good luck 1. If a 21.00 gram sample of a Cu-Zn-Ni alloy contains 7.75 g Cu and 10.58 g Ni, what
More informationMULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question.
Exam Name MULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question. 1) What species is represented by the following information? 1) p+ = 17 n = 18 e- = 18 A)
More informationChapter How many grams of a 23.4% by mass NaF solution is needed if you want to have 1.33 moles of NaF?
Chapter 13 1. Which of the following compounds is a strong electrolyte? a. NH 4Cl b. NaCl c. NaC 2H 3O 2 d. HCl e. All of the above 2. A solution that is 13.58% by mass of sugar contains 13.75 grams of
More informationM = Molarity = mol solute L solution. PV = nrt % yield = actual yield x 100 theoretical yield. PM=dRT where d=density, M=molar mass
Solubility Rules: 1. Most nitrate salts are soluble. 2. Most salts of alkali metals and ammonium cations are soluble. 3. Most chloride, bromide and iodide salts are soluble. Exceptions: salts containing
More informationCHE 105 EXAMINATION II March 11, 2010 University of Kentucky Department of Chemistry
CHE 105 EXAMINATION II March 11, 2010 University of Kentucky Department of Chemistry READ THESE DIRECTIONS CAREFULLY BEFORE STARTING THE EXAMINATION! It is extremely important that you fill in the answer
More informationName: Date: 5. Which of the following formulas is not correct? A) ZnSO4 B) Ca(OH)2 C) NaS D) KF E) NH4Br. Page 1
Name: Date: 1. Which one of the following statements about atomic structure is false? A) The electrons occupy a very large volume compared to the nucleus. B) Almost all of the mass of the atom is concentrated
More information(B) K2O potassium dioxide. REASON: correct name for (A) would be magnesium chloride, (B) = potassium oxide, (C) = cobalt (II) chloride
PRACTICE CHEMISTRY EOC TEST 1. Which substance is a conductor of electricity? (A) NaCl(s) (B) NaCl(l) (C) C6H12O6(s) (D) C6H12O6(l) REASON: Conductors of electricity (electrolytes) must be ionic (metal
More information4. What is the mass of a mol sample of sodium hydroxide? A) g B) g C) g D) g E) g
Chem 101A Study Questions, Chapters 3 & 4 Name: Review Tues 10/4/16 Due 10/6/16 (Exam 2 date) This is a homework assignment. Please show your work for full credit. If you do work on separate paper, attach
More informationSpring Final Exam Review
Directions: Complete all of the following questions. Turn this in on the day of your final and you can earn up to 10 bonus points on your final. You must number and answer every questions on a separate
More information4. What is the mass of a mol sample of sodium hydroxide? A) g B) g C) g D) g E) g
Chem 101A Study Questions, Chapters 3 & 4 Name: Review Tues 10/02/18 Due 10/04/18 (Exam 2 date) This is a homework assignment. Please show your work for full credit. If you do work on separate paper, attach
More informationHEMISTRY 110 EXAM 3 April 6, 2011 FORM A When the path is blocked, back up and see more of the way. 1. A 250 L vessel is evacuated and then connected to a 50.0 L bulb with compressed nitrogen. The pressure
More informationCHE 105 Exam 2 Spring 2017
CHE 105 Exam 2 Spring 2017 Your Name: Your ID: Question #: 1 What is the chemical formula of chromium(iii) bromide? A. CrBr B. CrBr2 C. Cr2Br D. Cr3Br E. CrBr3 F. Cr2Br3 Question #: 2 What is the correct
More informationQuestions 1 13 cover material from Exam 1
Questions 1 13 cover material from Exam 1 1. Which intermolecular forces are present in H Te(l)? A. dispersion only C. dispersion, dipole-dipole, and hydrogen bonding B. dispersion and dipole-dipole D.
More informationX212F Which of the following is a weak base in aqueous solution? A) H 2 CO 3 B) B(OH) 3 C) N 2 H 4 D) LiOH E) Ba(OH) 2
PX212SP14 Practice Exam II / Spring 2014 1. Which of the following statements are characteristic of acids? 1. They are proton donors. 2. They react with bases to produce a salt and water. 3. They taste
More information2. If a gas is released in a reaction (ex: Hydrogen gas bubbles off), is it written as a reactant or a product?
PRE-AP CHEMISTRY SPRING FINAL EXAM REVIEW Name _ Period Exam Date 100% COMPLETION OF THIS REVIEW BY THE DAY OF YOUR FINAL EXAM WILL COUNT AS A 5 POINT BONUS ADDED TO YOUR FINAL EXAM SCORE. THERE WILL BE
More information6. Place the following elements in order of increasing atomic radii: Mg, Na, Rb, Cl.
CH141 Practice Problems/Practice Final Exam Page 1 of 12 Name: 1. What is the SO 4 2- concentration of a solution prepared by dissolving 3.00 g of Na 2 SO 4 in 1.00 L of water? 2. What is the hybridization
More informationThe chemical potential energy of a substance is known as its ENTHALPY and has the symbol H.
Enthalpy Changes The chemical potential energy of a substance is known as its ENTHALPY and has the symbol H. During chemical reactions, the enthalpy can increase or decrease. The change in enthalpy during
More informationCHEMISTRY 102A Spring 2012 Hour Exam II. 1. My answers for this Chemistry 102 exam should be graded with the answer sheet associated with:
. My answers for this Chemistry 0 exam should be graded with the answer sheet associated with: a) Form A b) Form B c) Form C d) Form D e) Form E. A sample of LSD (D-lysergic acid diethylamide, C 4 H 30
More informationCHEMISTRY 110 EXAM 3 Nov. 11, 2013 ORM A!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!" 1. The cylinder shown below is filled with enough N 2 gas at 25 o C to reach a
More informationAP Chapter 6: Thermochemistry Name
AP Chapter 6: Thermochemistry Name Warm-Ups (Show your work for credit) Date 1. Date 2. Date 3. Date 4. Date 5. Date 6. Date 7. Date 8. AP Chapter 6: Thermochemistry 2 Warm-Ups (Show your work for credit)
More informationCHEMISTRY Midterm #2 October 26, Pb(NO 3 ) 2 + Na 2 SO 4 PbSO 4 + 2NaNO 3
CHEMISTRY 123-02 Midterm #2 October 26, 2004 The total number of points in this exam is 100. The total exam time is 50 min. Good luck! PART I: MULTIPLE CHOICE (Each multiple choice question has a 2-point
More informationCHEM 1105 S10 March 11 & 14, 2014
CHEM 1105 S10 March 11 & 14, 2014 Today s topics: Thermochemistry (Chapter 6) Basic definitions Calorimetry Enthalpy Thermochemical equations Calculating heats of reaction Hess s Law Energy and Heat Some
More informationCHEMISTRY 110 EXAM 3 NOVEMER 12, 2012 FORM A
CHEMISTRY 110 EXAM 3 NOVEMER 12, 2012 FORM A 1. Consider a balloon filled with 5 L of an ideal gas at 20 C. If the temperature of the balloon is increased by 70 C and the external pressure acting on the
More information1) REACTIONs: a) Al4C3(s) + H2O (l)=> Al(OH)3 (s) + CH4 (g) Solution : Al4C3(s) + 12 H2O (l)=> 4Al(OH)3 (s) + 3CH4 (g)
1) REACTIONs: a) Al4C3(s) + H2O (l)=> Al(OH)3 (s) + CH4 (g) Balance the reaction. Describe the chemical process represented by this reaction. Write the name of each single reactant and product. First,
More information2. Remember the honor system. No notes, books, stored information in calculators, or external help is allowed.
Chem 5 Test #1 Fall 2003 Name General instructions: 1. Don t panic! Write down what you know and what you need to figure out. Think about all relevant equalities. Make sure to keep track of units. Check
More informationc. K 2 CO 3 d. (NH 4 ) 2 SO 4 Answer c
Chem 130 Name Exam 2, Ch 4-6 July 7, 2016 100 Points Please follow the instructions for each section of the exam. Show your work on all mathematical problems. Provide answers with the correct units and
More informationCHAPTER 11 Stoichiometry Defining Stoichiometry
CHAPTER 11 Stoichiometry 11.1 Defining Stoichiometry Stoichiometry is the study of quantitative relationships between amounts of reactants used and products formed by a chemical reaction. Stoichiometry
More informationChem 1100 Pre-Test 3. Multiple Choice Identify the choice that best completes the statement or answers the question.
Chem 1100 Pre-Test 3 Multiple Choice Identify the choice that best completes the statement or answers the question. 1. Determine the oxidation number of the underlined element in K 2CO 3. a. 1 b. 2 c.
More informationWorkbook 5. Chem 1A Dr. White 1
Chem 1A Dr. White 1 Workbook 5 5-1: Dalton s Law, KMT, Effusion/Diffusion/Real Gases 1. What is the total pressure and the partial pressure of each gas (in atm) in a mixture of 3.2 g of O 2, 1.6 g of CH
More informationAP Chemistry Semester 1 Practice Problems
AP Chemistry Semester 1 Practice Problems 1. Adipic Acid contains 49.32% C, 43.84% O, and 6.85% H by mass. What is the empirical formula? a) C 3 H 5 O 2 b) C 3 H 3 O 4 c) C 2 HO 3 d) C 2 H 5 O 4 e) C 3
More informationChemistry 116 Pre-test Some questions from Chem 115 Final exam; Fall 2014
1. The mass of a sample is 550 milligrams. Which of the following expresses that mass in kilograms? a. 5.5 10 8 kg b. 5.5 10 5 kg c. 5.5 10 4 kg d. 5.5 10 6 kg e. 5.5 10 1 kg 2. Select the answer that
More informationANSWERS CIRCLE CORRECT SECTION
CHEMISTRY 162 - EXAM I June 08, 2009 Name: SIGN: RU ID Number Choose the one best answer for each question and write the letter preceding it in the appropriate space on this answer sheet. Only the answer
More informationChemistry 101 Chapter 4 STOICHIOMETRY
STOICHIOMETRY Stoichiometry is the quantitative relationship between the reactants and products in a balanced chemical equation. Stoichiometry allows chemists to predict how much of a reactant is necessary
More informationHonorsChemistry 2nd Semester Review MULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question.
Exam Name HonorsChemistry 2nd Semester Review MULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question. 1) Which process releases energy? 1) A) bond formation
More information1. Which type of bond involves the transfer of electrons from one atom to another? A. Hydrogen bond C. Metallic bond B. Ionic bond D.
1. Which type of bond involves the transfer of electrons from one atom to another? A. Hydrogen bond C. Metallic bond B. Ionic bond D. Covalent bond 2. Ethene (C 2 H 4 ) and cyclohexane (C 6 H 12 ) have
More informationFor the entire exam, solutions are aqueous and T = 25 C unless stated otherwise. Questions 1 15 cover material from Exam 1.
For the entire exam, solutions are aqueous and T = 25 C unless stated otherwise. Questions 1 15 cover material from Exam 1. 1. What state of matter is described as follows? On the molecular level, the
More information4. Most chloride salts are soluble. Identify an exception to this generalization. a. FeCl2 b. CaCl2 c. MgCl2 d. PbCl2 e. BaCl2
1. Balance the chemical equation associated with the complete combustion of benzene (C6H6) in oxygen. How many moles of oxygen will be required to completely combust a 0.96 mole sample of benzene? C6H6
More informationChemistry 104 Final Exam Content Evaluation and Preparation for General Chemistry I Material
Chemistry 104 Final Exam Content Evaluation and Preparation for General Chemistry I Material What is 25 mph in mm s 1? Unit conversions What is 1025 K in o F? Which is larger 1 ft 3 or 0.1 m 3? What is
More informationFinal Exam Review Questions You will be given a Periodic Table, Activity Series, and a Common Ions Chart CP CHEMISTRY
Final Exam Review Questions You will be given a Periodic Table, Activity Series, and a Common Ions Chart CP CHEMISTRY Part A True-False State whether each statement is true or false. If false, correct
More informationCHEMISTRY 101 SPRING 2010 FINAL FORM B DR. KEENEY-KENNICUTT PART 1
NAME (Please print ) CHEMISTRY 101 SPRING 2010 FINAL FORM B DR. KEENEY-KENNICUTT Directions: (1) Put your name on PART 1 and your name and signature on PART 2 of the exam where indicated. (2) Sign the
More informationGeneral Chemistry Multiple Choice Questions Chapter 8
1 Write the skeleton chemical equation for the following word equation: Hydrochloric acid plus magnesium yields magnesium chloride and hydrogen gas. a HClO 4 + Mg --> MgClO 4 + H 2 b HClO 4 + Mg --> MgClO
More informationAP Chemistry Note Outline Chapter 4: Reactions and Reaction Stoichiometry:
AP Chemistry Note Outline Chapter 4: Reactions and Reaction Stoichiometry: Water as a solvent Strong and Weak Electrolytes Solution Concentrations How to Make up a solution Types of Reactions Introduction
More informationMULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question.
941_2nd Exam_941117 MULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question. 1) If the heat capacity of a ceramic cup is 0.820 J C-1, how much heat is required
More informationENTHALPY, ENTROPY AND FREE ENERGY CHANGES
ENTHALPY, ENTROPY AND FREE ENERGY CHANGES Refer to the following figures for Exercises 1-6. The lines on the vertical axis represent the allowed energies. Assume constant spacing between levels to determine
More informationChem 11 UNIT 3: STOICHIOMETRY Name:
Chem 11 UNIT 3: STOICHIOMETRY Name: Ms. Pirvu Period: Writing & Balancing Equations Chemical reactions can be described by chemical equations. Recall Law of Conservation of Mass mass cannot be nor. This
More informationChemistry Spring 2018 Final Exam Review
Name Date Period Chemistry Spring 2018 Final Exam Review TURN THIS COMPLETED REVIEW IN TO YOUR TEACHER BY DAY OF YOUR FINAL FOR A 5 point FINAL EXAM BONUS Unit #7 Moles 1. What is a mole? 2. What is molar
More informationSOLUTIONS - CHAPTER 9 Problems
SOLUTIONS - CHAPTER 9 Problems NOTE: Exam 3 will be on Tuesday, November 22 nd, from 8:30pm to 10:30pm. Room assignments for the exam are the same as for the first two exams. The exam will cover the following
More informationFACULTY OF SCIENCE MID-TERM EXAMINATION 2 MARCH 18, :30 TO 8:30 PM CHEMISTRY 120 GENERAL CHEMISTRY
FACULTY OF SCIENCE MID-TERM EXAMINATION 2 MARCH 18, 2011. 6:30 TO 8:30 PM CHEMISTRY 120 GENERAL CHEMISTRY Examiners: Prof. B. Siwick Prof. A. Mittermaier Dr. A. Fenster Name: Associate Examiner: A. Fenster
More informationCHEMpossible. 101 Exam 2 Review
CHEMpossible 1. Circle each statement that applies to thermal energy and heat: a. Thermal energy is the average kinetic energy of its molecules due to their motion b. High thermal energy is reflected in
More informationAcid Base Review. Page 1
1. Which substance, when dissolved in water, forms a solution that conducts an electric current? A) C2H5OH B) C6H12O6 C) C12H22O11 D) CH3COOH 2. A substance is classified as an electrolyte because A) it
More information